The solubility product of lead bromide is 8 t | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(D) Let the solubility of $PbBr_2$ be $S \ M$.The dissociation reaction is: $PbBr_{2(s)} \rightleftharpoons Pb^{2+}_{(aq)} + 2Br^-_{(aq)}$.Given the d

Vedclass · Accepted Answer

$3.4 	imes 10^{-2} \ M$

Vedclass · Answer

(D) Let the solubility of $PbBr_2$ be $S \ M$.The dissociation reaction is: $PbBr_{2(s)} ightleftharpoons Pb^{2+}_{(aq)} + 2Br^-_{(aq)}$.Given the degree of dissociation $\alpha = 0.8$,the concentrations of ions in the saturated solution are:$[Pb^{2+}] = \alpha S = 0.8S$$[Br^-] = 2 \alpha S = 2 	imes 0.8S = 1.6S$The solubility product expression is $K_{sp} = [Pb^{2+}][Br^-]^2$.Substituting the values: $8 	imes 10^{-5} = (0.8S) 	imes (1.6S)^2$.$8 	imes 10^{-5} = 0.8S 	imes 2.56S^2 = 2.048S^3$.$S^3 = \frac{8 	imes 10^{-5}}{2.048} \approx 3.906 	imes 10^{-5} = 39.06 	imes 10^{-6}$.$S = \sqrt[3]{39.06} 	imes 10^{-2} \approx 3.39 	imes 10^{-2} \ M \approx 3.4 	imes 10^{-2} \ M$.

The solubility product of lead bromide is $8 \times 10^{-5}$. If the salt is $80\%$ dissociated in a saturated solution,find the solubility of the salt.

Similar Questions

If the solubility product of $PbS$ is $3.4 \times 10^{-28}$,what is the minimum concentration of sulfide ions required to precipitate $PbS$ from a $0.001 \ M \ Pb^{2+}$ solution?

What is the minimum volume of water required to dissolve $1 \, g$ of calcium sulphate at $298 \, K$? (For calcium sulphate,$K_{sp}$ is $9.1 \times 10^{-6}$).

The solubility product constant $K_{sp}$ of $Mg(OH)_2$ is $9.0 \times 10^{-12}.$ If a solution is $0.010 \ M$ with respect to $Mg^{2+}$ ion,what is the maximum hydroxide ion concentration which could be present without causing the precipitation of $Mg(OH)_2$?

For $AgCl$,$K_{sp} = 1.2 \times 10^{-10}$ and for $AgBr$,$K_{sp} = 3.5 \times 10^{-13}$. What is the relationship between their solubilities $(S)$?

If the concentration of $[Ag^{+}]$ in a solution is $1 \times 10^{-6} \ M$,what is the concentration of $[Br^{-}]$? Given that the $K_{sp}$ for $AgBr$ is $4.0 \times 10^{-13}$.

Vedclass Test Series

Exam Paper Generator

Online Exam Module